Salts of sodium and potassium

Certain of the milk salts (e.g. chlorides, and the salts of sodium and potassium) are sufficiently soluble to be present almost entirely in the dissolved phase. The concentration of others, in particular calcium phosphate, is higher than can be maintained in solution at the normal pH of milk. Consequently, these exist partly in soluble form and partly in an insoluble or colloidal form associated with casein. The state and distribution of these salts has been extensively reviewed by Pyne (1962) and Holt (1985). 

The salts of sodium and potassium have been used for thousands of years in making soap and glass and for a great, number of other purposes. 

The black liquor used in this research work comes from the soda pulping of straw. The main components of these black liquor are three organic compounds, which come from the straw solution during the pulping, inorganic salts of sodium and potassium, and water. Moreover, it is important to indicate that the content of carbonates can reach 4.87 % wt. 

Clear evidence for this phenomenon has been established by D. Haynes and B. C. Pressman121b The selectivity of valinomycin with respect to Rb+, for instance, changes (cf. Table 3) from 0,60 to 2,75 (as expressed by ratios of stability constants relative to K+, for which the selectivity number is unity) when transferred from a solvent mixture of 70% toluene and 30% n-butanol to a medium containing 56% toluene and 44% n-butanol. Another example is the reversal of selectivity of dibenzo-18-crown-6 for the fluoryl salts of sodium and potassium. The sodium over potassium selectivity in tetrahydrofurane switches in oxetane to potassium over sodium as reported by K. W. Wonget al.3l2 ... 

Figure 6-11 shows Ce02 nanoparticles synthesized by this technique at 1073 K with the addition of the eutectic salts of sodium and potassium nitrate to the precursor solution prior to the aerosol decomposition [89]. The particles are composed of isolated nanoparticles whose mean size was 51 nm. 

The alkali metal tetrahydridoborates are salts those of sodium and potassium are stable in aqueous solution, but yield hydrogen in the presence of a catalyst. They are excellent reducing agents, reducing for example ion(III) to iron(II). and silver ions to the metal their reducing power is used in organic chemistry, for example to reduce aldehydes to alcohols. They can undergo metathetic reactions to produce other borohydrides, for example... 

An alloy of sodium and potassium (NaK) is used as a heat-transfer medium. Many potassium salts are of utmost importance, including the hydroxide, nitrate, carbonate, chloride, chlorate, bromide, iodide, cyanide, sulfate, chromate, and dichromate. 

Phenol s chemical properties are characterized by the influences of the hydroxyl group and the aromatic ring upon each other. Although the stmcture of phenol is similar to cyclohexanol, phenol is a much stronger acid. Its piC in aqueous solution at 25°C is 9.89 x 10 ° (8). This characteristic allows aqueous hydroxides to convert phenol into their salts. The salts, especially those of sodium and potassium, are converted back into phenol by aqueous mineral acids or carboxyhc acids. 

Some reactors are designed specifically to withstand an explosion (14). The multitube fixed-bed reactors typically have ca 2.5-cm inside-diameter tubes, and heat from the highly exothermic oxidation reaction is removed by a circulating molten salt. This salt is a eutectic mixture of sodium and potassium nitrate and nitrite. Care must be taken in reactor design and operation because fires can result if the salt comes in contact with organic materials at the reactor operating temperature (15). Reactors containing over 20,000 tubes with a 45,000-ton annual production capacity have been constmcted. 

Because of its functionaUty and environmental acceptabiUty, citric acid and its salts (primarily sodium and potassium) are used in many industrial appbcations for cbelation, buffering, pH adjustment, and derivatization. These uses include laundry detergents, shampoos, cosmetics, enhanced oil recovery, and chemical cleaning. 

Discussion. The method is applicable to the determination of a mixture of two salts having the same anion (e.g. sodium chloride and potassium chloride) or the same cation (e.g. potassium chloride and potassium bromide). For example, to determine the amount of sodium and potassium chlorides in a mixture of the two salts, a known weight (Wj g) of the solid mixture is taken, and the total chloride is determined with standard 0.1 M silver nitrate, using Mohr s method or an adsorption indicator. Let w2 g of silver nitrate be required for the complete precipitation of Wj g of the mixture, which contains xg of NaCl and yg of KC1. Then ... 

Salts of monovalent metals of alcohol and alcohol ether sulfates are soluble in water, with the solubility dependend on the cation and the chain length. Ammonium salts are more soluble than sodium salts and these are more soluble than potassium salts. On the other hand, sulfates with short hydrophobic chains are more soluble than those with longer chains but the short-chain molecules have a solubilizing effect on the more insoluble longer chain molecules [68], The solubility of sodium salts of different alcohol sulfates is shown in Fig. 2 and the solubility of sodium and potassium salts of dodecyl sulfate is compared. 

The alkaline product from the wood ash was a crude solution of sodium and potassium carbonates called "lye". On boiling the vegetable oil with the lye, the soap (sodium and potassium salts of long chained fatty acids) separated from the lye due to the dispersive interactions between the of the fatty acid alkane chains and were thus, called "lyophobic". It follows that "lyophobic", from a physical chemical point of view, would be the same as "hydrophobic", and interactions between hydrophobic and lyophobic materials are dominantly dispersive. The other product of the soap making industry was glycerol which remained in the lye and was consequently, termed "lyophilic". Thus, glycerol mixes with water because of its many hydroxyl groups and is very polar and hence a "hydrophilic" or "lyophilic" substance. 

Atomic hydrogen is a powerful reducing agent, even at room temperature. For example, it reacts with the oxides and chlorides of many metals, including silver, copper, lead, bismuth, and mercury, to produce the free metals. It reduces some salts, such as nitrates, nitrites, and cyanides of sodium and potassium, to the metallic state. It reacts with a number of elements, both metals and nonmetals, to yield hydrides such as NH3, NaH, KH, and PH3. Sulfur forms a number of hydrides the simplest is H2S. Combining with oxygen, atomic... 

Moltox A process for separating oxygen from air by selective absorption in a molten salt mixture at high temperature. Invented by D. C. Erickson of Energy Concepts, and developed by Air Products and Chemicals. The salts are a mixture of the nitrites and nitrates of sodium and potassium. The reaction is ... 

The electrolysis of aqueous solutions may not yield the desired products. Sir Humphry Davy (1778-1829) discovered the elements sodium and potassium by electrolyzing their molten salts. Before this discovery, Davy had electrolyzed aqueous solutions of sodium and potassium salts. He had not succeeded in reducing the metal ions to the pure metals at the cathode. Instead, his first experiments had produced hydrogen gas. Where did the hydrogen gas come from ... 

The results obtained with ISEs have been compared several times with those of other methods. When the determination of calcium using the Orion SS-20 analyser was tested, it was found that the results in heparinized whole blood and serum were sufficiently precise and subject to negligible interference from K and Mg ([82]), but that it is necessary to correct for the sodium error, as the ionic strength is adjusted with a sodium salt [82], and that a systematic error appears in the presence of colloids and cells due to complexa-tion and variations in the liquid-junction potential [76]. Determination of sodium and potassium with ISEs is comparable with flame photometric estimation [39, 113, 116] or is even more precise [165], but the values obtained with ISEs in serum are somewhat higher than those from flame photometry and most others methods [3, 25, 27, 113, 116]. This phenomenon is called pseudohyponatremia. It is caused by the fact that the samples are not diluted in ISE measurement, whereas in other methods dilution occurs before and during the measurement. On dilution, part of the water in serum is replaced by lipids and partially soluble serum proteins in samples with abnormally increased level of lipids and/or proteins. 

An interesting but still unexplained case refers to nitrobenzene. The reversible electron exchange between nitrobenzeneand sodium salt of the nitrobenzene- N anion-radical is characterized by the usual constant of 0.40. Stevenson et al. (1987b) used NH3(liq) as a solvent for these measurements at -75°C. Under the same conditions, they obtained the equilibrium constant of 2.1( ) for the electron exchange between nitrobenzene- N and the potassium salt of nitrobenzene- " N anion-radical. Perhaps, the difference between ion radii of sodium and potassium cations is crucial for the stability of the corresponding ion pair with nitrobenzene anion-radical. Such diversity can be pivotal when the electron prefers the heavy or light nitrobenzene. 

Treatment of sodium and potassium nitronates with alkyl halides typically results in the formation of oximes and carbonyl compounds by cleavage of the N—O bond (11). In one case, however, reaction of w-butyl bromide with the potassium salt of nitro ester 191 does afford the -butyl nitronate (192, Eq. 2.14) (154). 

The Stassfurt deposits have been the subject of elaborate investigations by J. H. van t Hoff and his school.16 In 1849, J. Usiglio 17 studied the deposition of salts when sea.water is cone, by evaporation, and examined the residues analytically. He found that calcium carbonate was first eliminated, then calcium sulphate, then sodium chloride, and the more soluble salts accumulated in the mother liquid. This method of investigation does not allow sufficient time for the various salts to attain a state of equilibrium, and it therefore follows that the natural evaporation of brines probably furnishes somewhat different results. Moreover, it is difficult, if not impossible, to identify the several substances which separate from the mother liquid formed during the later stages of the evaporation. J. H. van t Hoff followed the synthetic method in his study of this subject. He started from simple soln. like those of sodium and potassium chlorides, under definite conditions of temp., and gradually added the pertinent constituents until the subject became so complicated that the crystallization of the constituents from concentrating sea water was reduced to a special case of a far more comprehensive work. 

The equilibrium curve of mixtures of sodium and magnesium sulphates in aq. soln. for temp, up to just over 100°, is represented by Eig. 3. Below 22°, the case i3 analogous with mixtures of sodium and potassium chlorides, Eig. 1 (1.11,1), for sodium or magnesium sulphate alone crystallizes from the soln. as illustrated by the set of curves A1 at 22° A2, the double salt astracanite appears, and at higher temp., the zone of stability of astracanite widens as shown by the portions of the curves A3 and A4 between the dotted lines of the diagram. No astracanite separates from a sat. soln. of the two sulphates if the temp, is below 22°,... 

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